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Using the values of Delta H and Delta S given, calculate Delta G for each of the reactions at 25 degree C and indicate whether the reactions are spontaneous or non-spontaneous. Explain. Delta H = 10.5 kJ/mol and Delta S = 30.0 J/K-mol Delta H = -10.5 kJ/mol and Delta S = 105. J/K-mol
8.) From the values of delta H and delta S, calculate delta G then predict whether the following reactions would be spontaneous or not at 25 C. a) Reaction A: delta H= 10.5 kJ/mol, and delta S = 30 J/K mol b) Reaction B: delta H=1.8 kJ/mol, and delta S = -113 J/K mol 9.) Calculate the delta G and K, for the following equilibrium reaction at 25 C: 2H2O(Ⓡ) <-> 2H2(g) + O2(8) delta Gran H2O(x) = -228.6 kJ/mol
Use the Delta H degree_f and Delta H degree_rxn information provided to calculate Delta H degree_f for SO_3 (g): Delta H degree_f (kJ/mol)SO_2(g) + O_2(g) rightarrow SO_3 (g) Delta H degree_rxn = -198 kJ SO_2(g) - 297
assuming the values of delta H and delta S are constant, at what temperature does the reaction become nonspontaneous? Moving to the next question prevents changes to this answer Question 4 stion 14 3 points Sve The reaction PC3(E) + Cl28) PCi5(e) has a AS of vßon:-170.2 J/mol.K and a AH of -87.9 kJ/mol. Assuming the values of AH and As are constant, at what temperature does the reaction become to-spowaneous? 789.6°C 516.5°C 1863.3°C 243.3°C A ng to t o...
Use the Delta H degree_1 provided to calculate Delta H degree_rxn for the following: + 161 kJ -422 kJ + 800 kJ -256 kJ -62 kJ
Here are the delta H, delta S and delta G values from my textbook: (first value is delta H, second value is delta S, third is delta G) CO2: -393.5 , 213.6 , -394.4 CH4: -75, 186, -51 CO : -110.5 , 197.9 , -137.3 CH3COOH : -484.2 , 159.8 , -389.45 CH3OH : -238 , 126.8 , -166.3 Q3. Using the thermodynamics data given in the appendix, calculate ΔH·AS) and ΔG, for the following reactions that produce acetic acid:...
calculate the delta h,delta s and delta s universe for this reaction. determine the spontaneity of the reaction. Question 7 KO2(g) + H2(g) = H2O(g) Calculate the AH, AS and AS universe for this reaction. Determine the spontaneity of the reaction. AHAG So Substance kJ/mol kJ/mol J/(mol-K) 1 0 Ag S Agt(a) AgBr(s) Agcls Agls) Cl2(g) Cl(g Cl(aq) Br-fag) H+ (aq) Hz(g) H2O(g) H2O(0 H3O+ (aq) H20200 HBr(g) HCl(g) HCN(g) KS Kag) KO2(aq) KOHS) KBr(s) KCIS KCIO3(s) 0(8) O2(g) 03(g)...
how can i find the delta h of the reaction and the average delta h of the reacting in kj? Chemistry 1A Name Lab Partner Trial 1 Trial 2 Calorimeter Constant (Cel) from Part 1 - 462 Grın (heat released by reaction, in J) = AH =(heat absorbed by mixture + Cat AT) show calculations 103 6.35 + (-462/c- 9.4°c). cran : AM. - 3306,5 J - 2306.55 Moles of metal used. show calculations 0.4397n ( stan): 0.00066 mol en...
From the values of delta H and delta S, predict which of the following reactions would be spontaneous at 26C: Reaction A: delta H = 10.5 kJ/mol, delta S = 30.0 J/K*mol Reaction B: delta H = 1.8 kJ/mol, delta S = -113 J/K*mol If either of the reactions is nonspontaneous, can it (they) become spontaneous? If either of the reactions is nonspontaneous but can become spontaneous, at what temperature might it become spontaneous? Please explain how to do this!
How to calculate heat release given moles of precipitate and delta H of the reaction? Ex: if the Delta H reaction =-55.5kJ, how much heat is released when 3.31 moles of precipitate are formed?